1. OXYGEN OXYGEN AND ITS PROPERTIES

2. By the end of this presentation you should be able to: Demonstrate an understanding of how to investigate the proportion of oxygen in the atmosphere

3. The amount of oxygen in the atmosphere depends on where you sample it from. The higher you go the less there is! In this lesson we will find the percentage of oxygen in the atmosphere in our laboratory… 500 feet above sea-level!

4. Strategy… Trap a known amount of air; a cm 3 Remove the oxygen! Measure the amount of ‘air’ left ; b cm 3 Calculate amount of oxygen removed Calculate the percentage of oxygen; a – b a x 100 a – b cm 3

5. Copper + oxygen  copper oxide The oxygen in the atmosphere can be removed by passing a sample of the atmosphere over hot copper. If copper is heated in air, the hot copper combines with the oxygen, to form… and so removes it from the air. solid copper oxide… 2Cu (s) + O 2 (g)  2CuO (s) +  Remove the oxygen!

7. The experiment… Two gas syringes are joined together with one containing a known volume of air, 100 cm 3, and the other empty. 100 cm 3 Copper turnings are put in a combustion boat such that the air can be pushed over them. The copper turnings are heated. (a cm 3 )

8. The air is passed to and fro over the copper to allow the hot copper to react. The copper goes darker as copper oxide is formed. The experiment…

9. The apparatus is allowed to cool and the volume of gas remaining in the syringe is measured. 79 cm 3 The volume of oxygen is calculated by taking the final volume from the original volume… The experiment… (b cm 3 )

10. The apparatus is allowed to cool and the volume of gas remaining in the syringe is measured. 79 cm 3 The calculation… (b cm 3 ) ( a cm 3 ) ( a – b ) cm 3 ( a cm 3 ) 100 cm 3 a – b a x 100 = 21%

11. Possible errors… 79 cm 3 There is some air in the tube with the copper turnings. The oxygen in this air will also react with the hot copper, causing a small error in the final volume recorded. Since gases occupy greater volumes when hot… …it is important to let the apparatus cool down at the end of the experiment otherwise the final reading will be too high… The initial volume and the final volume must be measured at the same temperature.

14. Laboratory Preparation of Oxygen Oxygen is prepared in the lab by catalytic decomposition of hydrogen peroxide using manganese (IV) oxide as shown. The gas is then collected over water.

16. Separation of Oxygen and Nitrogen from Air 1.Air is a mixture and its components can be separated by processes involving physical changes. 2.Components in air such as oxygen, nitrogen and noble gases have many uses, therefore it is important to obtain them separately. 3.In industry, the components of air can be separated by fractional distillation of liquid air. This is possible because different components in air have different boiling points.

17. air in nitrogen gas (b.p. -196 o C) argon gas (b.p. -186 o C) oxygen gas (b.p. -183 o C) 1 2 3 4

18. (i)Purification 1. Dust particles are removed by filter. 2. Water vapour and carbon dioxide are removed as solids at -80 o C (ii)Liquefaction of air 3. Air is compressed and then cooled. 4. Air is then allowed to expand - it gets very cold and becomes liquid at -200 o C.

19. (iii)Fractional distillation of liquid air The liquid air is pumped into a fractionating tower and then allowed to warm up very slowly. Different gases in liquid air boil at their own boiling points, so they can be collected one by one. The boiling point of nitrogen is -196 o C and it boils off first and is collected at the top of the fractionating tower. Argon follows (boiling point -186 o C) and then oxygen (boiling point -183 o C) which is collected at the lower part of the fractionating tower.

20. The boiling points of some of the gases found in air are in shown in the table below. GasBoiling point ( o C) Argon -186 Nitrogen-196 Neon-246 Oxygen-183 Helium-269 Krypton-153

21. (VI) Uses of gases in air Oxygen – in breathing Carbon dioxide – in fire extinguisher Dry ice (solid carbon dioxide) is used in refrigeration Helium – filling balloons Argon – filling light bulbs

22. Properties of Oxygen

23. Carbon Burns in Oxygen

24. Properties of Oxygen

25. Chemical test for Oxygen A glowing match or wooden splint will relight when placed in oxygen gas.

26. To Show That Air contains Carbon Dioxide and Water Vapour

28. RUSTING OF IRON

29. Experiment 1.Place the painted nail in a test tube and totally cover with water – label this painted nail + water 2.Put a plain nail in a test tube and ½ cover this with water – label this control 3.Cover a plain nail in Vaseline (using a paper towel) and totally cover with water – label this greased nail 4.Add some calcium chloride crystals in a test tube, and add a little cotton wool in the top of the test tube, pushing it down with a spatula so that it is just above the crystals. Add a plain nail on top of the cotton wool, and place some more cotton wool in the top of the test tube – label this calcium chloride 5.Put a plain nail in a test tube and totally cover this with boiled water. Add a little oil on top of the water, and bung the test tube – label this oil 6.Label your test tube with your group names

33. Combustion is the chemical reaction that takes place when a substance burns. The substance reacts with oxygen and energy is released as heat and light. Combustion is an important reaction as more than 90% of the world’s energy comes from burning fossil fuels like coal, natural gas and petrol. Where do fossil fuels come from and what other fuels are there? Using combustion

34. Incomplete combustion A good supply of oxygen is needed for a fuel to burn completely and release as much energy as possible. When carbon reacts completely with oxygen, it is all turned into carbon dioxide. This is called complete combustion: carbon dioxide oxygen carbon If there is not enough oxygen, a fuel cannot burn completely and less energy is released. Some fuel is wasted. When carbon does not react completely with oxygen, the product is carbon monoxide, a colourless poisonous gas. This is called incomplete combustion: carbon monoxide oxygen carbon

35. Demonstration – Burning magnesium in the air Wear eye protection. 1.Watch what happens when your teacher burns magnesium in air. 2.Describe what you see. 3.What element present in the air reacted with the magnesium? 4.Describe the product formed. 5.What is the name of this product?

36. Demonstration – Burning magnesium in the air Wear eye protection. 1.Watch what happens when your teacher burns magnesium in air. 2.Describe what you see. 3.What element present in the air reacted with the magnesium? 4.Describe the product formed. 5.What is the name of this product?

37. Experiment - Investigating the reaction between magnesium and oxygen Wear eye protection. Method 1.Place the strip of magnesium ribbon into the crucible and put on the lid. 2.Using the electronic scales, weigh the crucible (including the lid) and magnesium and record the mass. 3.Heat the crucible strongly, once the magnesium begins burning, use tongs, to lift up the lid to let some air in. Try not to let any smoke out. 4.When there is no further change to the magnesium, turn off the Bunsen burner and leave the crucible for 10 - 15 minutes to cool. 5.Draw a labelled diagram of the apparatus, and write the method in the past tense (A strip of magnesium was ….). 6.When the crucible is cool to the touch re-weigh it with its lid. 7.Explain the change in mass.

38. crucible and lid pipe clay triangle tripodbunsen burner heat proof mat Write the word equation for the reaction. magnesium + oxygen magnesium oxide Experiment - Investigating the reaction between magnesium and oxygen

39. Why did the mass increase in the crucible? magnesium + oxygen magnesium oxide Mg O O O O 2Mg + O 2 2MgO What was present in the crucible when it was first weighed? What was present in the crucible at the end of the experiment? Write your explanation.

40. Competition for Oxygen

41. Solid copper(II) oxide can be reduced by passing a stream of hydrogen gas over the heated solid.

42. Write a balanced symbol equation for the reaction between copper(II) oxide and hydrogen gas. What would you observe during this reaction?

43. Write a balanced symbol equation for the reaction between copper(II) oxide and hydrogen gas. CuO + H 2 → Cu + H 2 O What would you observe during this reaction? Black solid turns pink/brown flame diminishes in size drops of colourless liquid appear at cooler parts.

45. The Reaction Between Magnesium and CO 2

48. Air Pollution

49. Air pollution is the presence of substances in the air that are harmful to health or the environment. It can be easy to spot air pollution in cities, but its effects are not limited to urban areas because air circulates freely all over the world. Air pollution can cause the destruction of forests, death of fish in lakes and premature death in humans. How does air pollution cause so many problems?

50. The most common pollutants found in air are: carbon dioxide (CO 2 ) sulphur dioxide (SO 2 ) carbon monoxide (CO) nitrogen dioxide (NO 2 ) All these gases emanate from burning substances in Oxygen

51. Carbon dioxide is an important atmospheric gas as it prevents heat radiation produced by the Earth from escaping into space. This is the greenhouse effect, which makes the Earth warm enough for life. Fossil fuels often contain sulphur and so the pollutant sulphur dioxide can be produced during combustion. If there is not enough oxygen present when fossil fuels are burned, incomplete combustion occurs. This reaction produces carbon and carbon monoxide gas.

52. Carbon monoxide gas is extremely harmful to human health because it stops blood from carrying oxygen.